A.) What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver nitrate is added to 1.00 L of solution that is 1.080 M in CN-. For [Ag(CN)2]-, Kf = 1.3×1021. B.) What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00×10-2 mol zinc nitrate is added to 1.00 L of solution that is 1.080 M in OH-. For [Zn(OH)4]2-, Kf = 4.6×1017.
A.) What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver nitrate is added to 1.00 L of solution that is 1.080 M in CN-. For [Ag(CN)2]-, Kf = 1.3×1021. B.) What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00×10-2 mol zinc nitrate is added to 1.00 L of solution that is 1.080 M in OH-. For [Zn(OH)4]2-, Kf = 4.6×1017.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter17: Solubility And Complex-ion Equilibria
Section: Chapter Questions
Problem 17.103QP: Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia....
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A.) What is the approximate concentration of free Ag+ ion at equilibrium when 1.43×10-2 mol silver nitrate is added to 1.00 L of solution that is 1.080 M in CN-. For [Ag(CN)2]-, Kf = 1.3×1021.
B.) What is the approximate concentration of free Zn2+ ion at equilibrium when 1.00×10-2 mol zinc nitrate is added to 1.00 L of solution that is 1.080 M in OH-. For [Zn(OH)4]2-, Kf = 4.6×1017.
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